Chemical engineering - process design, coursework, Other Subject

ProblemStyrene can be produced by the reactions:Ethylbenzene ! Styrene+H2Ethylbenzene ! Benzene+EthyleneEthylbenzene+H2 ! Toluene+CH4The reactions take place at 600C and 1.7 bar. We want to produce 100 molh of styrene. The market pricesare 22 Â£/mol for styrene, 10 Â£/mol for benzene and 7 Â£/mol for toluene. The ethylbenzene feed streamcontains 2% benzene and costs 16 Â£/mol. Fuel price is Â£10 for 106 cal. Assume that fuel componentshave normal boiling points larger than 50C. For the product distribution, the following correlations havebeen determined experimentally by chemists:mol Benzenemol Styrene = 0:333x??0:215x2+2:547x3mol Toluenemol Styrene = 0:084x??0:264x2+2:638x3where x is the ethylbenzene conversion.Determine and justify the following decisions (remember: think as an engineer!):1. Should the above process be continuous or batch?2. Based purely on the level 0 information, what is a reasonable upper bound on the conversion weshould consider?3. Do we need feed purification?4. Do we use gas recycle and purge stream(s)?5. What is the number of product streams?6. Draw the input-output flowsheet.7. Develop the overall material balances for the input-output structure as a function of the clearly identifieddesign variable(s).8. Plot the economic potential as a function of the design variables.9. Above what conversion does the above process become unprofitable?10. Produce a stream table for what you would consider to be a good conversion.